bonding and inorganic nomenclature
DESCRIPTION
lithium nitrate. lead (II) sulfide. barium sulfide. lithium nitride. Chemistry. sulfur dioxide. lithium nitrite. Bonding and Inorganic Nomenclature. NO 2. NaClO 3. N 2 O 4. Fe(ClO 3 ) 2. N 2 O 5. Fe(ClO 3 ) 3. potassium nitrate. copper (II) sulfate. sodium hydroxide. KNO 3. - PowerPoint PPT PresentationTRANSCRIPT
Bonding andInorganic Nomenclature
Chemistry
NaClO3
Fe(ClO3)2
lithium nitrate
lithium nitride
lithium nitrite
lead (II) sulfide
barium sulfide
sulfur dioxide
Fe(ClO3)3
NO2
N2O4
N2O5
Inorganic Nomenclature
potassiumnitrateKNO3
sodiumhydroxide
NaOH
dinitrogen monoxideN2O
copper (II)sulfate
Cu2SO4
Vocabulary
• Chemical Bond
– attractive force between atoms or ions that binds them together as a unit
– bonds form in order to…• decrease potential energy (PE)
• increase stability
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Covalent Bonding - True Molecules
Types of Bonds
Diatomic Molecule
Ammonia
Nitrogen
Water
In insulators (like wood),the v.e– are attachedto particular atoms.
Metallic Bonds
In metals, valence shells of atoms overlap, so v.e– are free to travel between atoms through material.
Not so in metals.
All due to free-moving
v.e–.
Properties of Metals
ductile conduct heat and electricity
malleable
Ionic Bonding - Crystal Lattice
Types of Bonds
Table salt
Properties of Salts
1. very hard –
2. high melting points –
3. brittle –
each ion is bondedto several oppositely-charged ions
many bonds must be broken
with sufficient force,like atoms arebrought next toeach other and repel
calcite
Chemical Bonding
Ionic Bonds: atoms give up or gain e– and are attracted to each other by coulombic (electrical) attraction
Na Na1+ Cl Cl1–loses e– gains e–
Na1+ + Cl1– NaCl
K1+ + NO31– KNO3
ionic compounds = salts
where NO31– is a polyatomic ion:
a charged group of atoms that stay together
Writing Formulas of Ionic Compounds
chemical formula:
To write an ionic compound’s formula, we need:
1. the two types of ions
2. the charge on each ion
Na1+ and F1–
Ba2+ and O2–
Na1+ and O2–
Ba2+ and F1–
shows types of atomsand how many of each
NaF
BaO
Na2O
BaF2
(i.e., “pink” and “blue”)
has neutral charge;
charge on cation / anion“becomes” subscript of anion / cation
** Warning:
Al3+ and O2– Ba2+ and S2– In3+ and Br1–
Reduce to lowest terms.
Al O Ba S In Br 2 3 2 2 31
Al2O3 BaS InBr3
criss-cross rule:
Writing Formulas w/Polyatomic Ions
Parentheses are required only when you need morethan one “bunch” of a particular polyatomic ion.
Ba2+ and SO42–
Mg2+ and NO21–
NH41+ and ClO3
1–
Sn4+ and SO42–
Fe3+ and Cr2O72–
NH41+ and N3–
BaSO4
Mg(NO2)2
NH4ClO3
Sn(SO4)2
Fe2(Cr2O7)3
(NH4)3N
A. To name, given the formula:
2. Use name of anion (it has the ending “ide”).
1. Use name of cation.
NaF
BaO
Na2O
BaF2
sodium fluoride
barium oxide
sodium oxide
barium fluoride
Na
Ba
1. Write symbols for the two types of ions.
2. Balance charges to write formula.
silver sulfide
zinc phosphide
calcium iodide
B. To write formula, given the name:
Ag1+ S2– Ag2S
Zn2+ P3– Zn3P2
I1– Ca2+ CaI2
CaAg
Zn
Ionic Compounds (cation/anion combos)
The Unique-Charge Cations (Always have the same charge when ionized)
The unique-charge cations are:
groups 1, 2, 13, and Ag1+, Cd2+, and Zn2+ 1
2 13
Variable-Charge Cations with Elemental Anions
The Variable (multiple)-charge cations are:
Pb, Sn, and the transition elements
Ag Cd
Zn
(but – not Ag+1, Cd+2, or Zn+2)
iron oxide
A. To name variable charge elements, given the formula:
1.Figure out charge on cation.2. Write name of cation.
3. Write Roman numerals in ( ) to show cation’s charge.
4. Write name of anion.
FeO
Fe2O3
CuBr
CuBr2
iron oxide
CuFe
Stock Systemof nomenclature
Fe? O2– iron (II) oxide
Fe? O2– iron (III) oxide
copper bromide
copper bromide
Cu? Br1– copper (I) bromide
Cu2+ Br1– copper (II) bromide
Fe?
Br1–
O2– O2–
Fe2+
Fe3+ Fe3+
Cu1+
Cu?
B. To find the formula, given the name:
1. Write symbols for the two types of ions.
2. Balance charges to write formula.
cobalt (III) chloride
tin (IV) oxide
tin (II) oxide
Co
Sn
Co3+ Cl1– CoCl3
Sn4+
O2–
O2–
Sn2+
SnO2
SnO
Compounds Containing Polyatomic Ions
Insert name of ionwhere it should goin the compound’sname.
Write formulas:
iron (III) nitrite
ammonium phosphide
ammonium chlorate
zinc phosphate
lead (II) permanganate
iron (III) nitrite
ammonium phosphide
ammonium chlorate
zinc phosphate
lead (II) permanganate
Fe3+ NO31– Fe(NO3)3
NH41+
NH41+
P3– (NH4)3P
ClO31– NH4ClO3
Zn2+ PO43– Zn3(PO4)2
Pb2+ MnO41– Pb(MnO4)2
Write names:
(NH4)2S2O3
AgBrO3
(NH4)3N
U(CrO4)3
Cr2(SO3)3
(NH4)2S2O3
AgBrO3
(NH4)3N
U(CrO4)3
Cr2(SO3)3
ammonium thiosulfate
silver bromate
ammonium nitride
U? CrO42–
CrO42–
CrO42–
uranium (VI) chromate
Cr? Cr?
Cr3+ Cr3+ SO3
2– SO32–
SO32– chromium (III) sulfite
U6+
Binary Molecular Compounds(Covalent Compounds)
Nonmetal + Nonmetal
Covalent Bonds
…atoms share e– to get a full valence shell
Lewis structure:
1. Two shared e– make a single covalent bond,four make a double bond, etc.
2. unshared pairs: pairs of unbonded valence e–
3. Each atom needs a full outer shell, i.e., 8 e–.
Exception: H needs 2 e–
a model of a covalent molecule that
shows all of the valence e–
Group 14 (4 v.e–)
Group 17 (7 v.e–)
both need 8 v.e– for a full outer shell (octet rule)
C
F
x
x
H
x x
xx
x xF x
carbon tetrafluoride (CF4)
o
Co
o o
x
xxx
x xF x
o
Co
o ox
xxx
x xF x
x
xxx
xF x
x
xxx
x xF x
x
x
xxx
x xF x
x
xxx
x xF x
x
xxx
x xF x
methane (CH4)
o
Co
o o
H x
o
Co
o oH x
xH
x H
H x
H x
H x
ooo
oN o
nitrogen triiodide (NI3)
carbon dioxide (CO2)
x x
xx
x x I x
x
xxx
x x I x
x
xxx
x x I x
xxx
x x I x
x
x
xxx
x x I x
x
xxx
x x I xoo
o
oN o
o
Co
o o x
xxx
xO x
x
xxx
xO x
x
xxx
xO x
o
Co
o o O = C = O
x x
x x x x
x x
x
xxx
xO x
butter
(consist of twononmetal elements)
covalent compounds = molecular compounds
-- have lower melting points than do ionic compounds
mono
Covalent Compounds -- contain two types of
** Key:
Use Greek prefixes to indicate howmany atoms of each element, butdon’t use “mono” on first element.
nonmetals nonmetals
FORGET CHARGES!
What to do:
1 –2 –
3 –
4 –
5 –
6 –7 –
8 –
9 –
10 –
di
tri
tetra
penta
hexa
hepta
octa
nona
dec
EXAMPLES:
carbon dioxide
CO
dinitrogen trioxide
N2O5
carbon tetrachloride
NI3
CO2
carbon monoxide
N2O3
dinitrogen pentoxide
CCl4
nitrogen triiodide
Binary Compounds Containing Two Nonmetals
To name these compounds, give the name of the less electronegative element first with the Greek prefix indicating the number of atoms of that element present, followed by the name of the more electronegative non-metal with the Greek prefix indicating the number of atoms of that element present and with its ending replaced by the suffix –ide.
Prefixes you should know:
Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca
1 2 3 4 5 6 7 8 9 10
Dihydrogen Monoxide:A Tale of Danger and
Irresponsibility
-- major component of acid rain
-- found in all cancer cells
-- inhalation can be deadly
-- excessive ingestion results in acute physical symptoms:
e.g., frequent urination, bloated sensation, profuse sweating
-- often an industrial byproduct of chemical reactions; dumped wholesale into rivers and lakes
Binary CompoundsContaining Two Nonmetals (Type III Compounds)
1. ________________ diarsenic trisulfide
2. ________________ sulfur dioxide
3. P2O5 ____________________
4. ________________ carbon dioxide
5. N2O5 ____________________
6. H2O ____________________
As2S3
SO2
diphosphorus pentoxide
CO2
dinitrogen pentoxide
dihydrogen monoxide
Binary Molecular Compounds
N2O dinitrogen monoxideN2O3 dinitrogen trioxideN2O5 dinitrogen pentoxide
ICl iodine monochlorideICl3 iodine trichloride
SO2 sulfur dioxideSO3 sulfur trioxide
Naming Binary CompoundsBinary Compound?
Metal Present?
Does the metal formmore than one cation?
Type IIIUse Greek
Prefixes
Type IUse the elementname for the cation.
Type IIDetermine the charge of the cation; use a Romannumeral after the cationname.
Yes
Yes
YesNo
No
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 98
Naming Simple Chemical Compounds
Ionic (metal and nonmetal) Covalent (2 nonmetals)
Metal
Formsonly onepositive
ion
Formsmore than
one positiveion
Nonmetal
Use the name of element
Use elementname followed
by a Romannumeral to
show the charge
Firstnonmetal
Secondnonmetal
Beforeelement name
use a prefixto matchsubscript
Use a prefixbefore
element name and end with ide
SingleNegative
Ion
Polyatomic Ion
Use the nameof the
element, butend with ide
Use thename of
polyatomicion (ate or
Ite)
Prefixes – Binary Molecular CompoundsGreek Prefixes for Two Nonmetals
Number Indicated Prefixes
1 mono- 2 di- 3 tri- 4 tetra- 5 penta- 6 hexa- 7 hepta- 8 octa- 9 nona-10 deca-
Page 131 in text
phosphate
sulfate
carbonate
chlorate
nitrate
Polyatomic Ions - Memorize
phosphATE
sulfATE
carbonATE
chlorATE
nitrATE
PO43- ……………
SO42- ……………
CO32- …………..
ClO31- …………..
NO31- ………..….
Eight “-ATE’s”
Exceptions:
ammonium
hydroxide
cyanide
NH41+ ……………
OH1- ……………
CN1- …………..
Pattern to Memorizing Nomenclature
XY“-ide”
XYO3“-ate”
XYO2“-ite”
XYO“hypo___-ite”
XYO4“per___-ate”
normal 1 less oxygen 2 less oxygen1 more oxygen
Polyatomic Ion: a group of atoms that stay together and have a single, overall charge.
BrO41-
Perbromate ion
BrO31-
Bromate ion
BrO21-
Bromite ion
BrO1-
Hypobromite ion
CO42- CO3
2-
Carbonate ion
CO22- CO2-
ClO41- ClO3
1-
Chlorate ion
ClO21- ClO1-
IO41- IO3
1-
Iodate ion
IO21- IO1-
NO41- NO3
1-
Nitrate ion
NO21- NO1-
PO53- PO4
3-
Phosphate ion
PO33- PO2
3-
SO52- SO4
2-
Sulfate ion
SO32- SO2
2-
1 more oxygen “normal” 1 less oxygen 2 less oxygen
Common Polyatomic Ions(pg 123 in text)
Names of Common Polyatomic Ions
Ion Name Ion Name
NH4 1+ ammonium CO3 2- carbonate
NO2 1- nitrite HCO3 1- hydrogen carbonate NO3 1- nitrate (“bicarbonate” is a widely SO3 2- sulfite used common name) SO4 2- sulfate ClO 1- hypochlorite HSO4 1- hydrogen sulfate ClO2 1- chlorite
(“bisulfate” is a widely ClO3 1- chlorate used common name) ClO4 1- perchlorate OH 1- hydroxide C2H3O2 2- acetate CN 1- cyanide MnO4 1- permanganate PO4 3- phosphate Cr2O7 2- dichromate HPO4 2- hydrogen phosphate CrO4 2- chromate H2PO4 1- dihydrogen phosphate O2 2- peroxide
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 100 Print Version
Binary Hydrogen Compoundsof Nonmetals When Dissolved in Water
(These compounds are commonly called acids.)
The prefix hydro- is used to represent hydrogen, followed by the nameof the nonmetal with its ending replaced by the suffix –ic and the wordacid added. (See page 133 in text for common acids)
Examples:
*HCl
HBr
*The name of this compound would be hydrogen chloride if it was NOT dissolved in water.
Hydrochloric acid
Hydrobromic acid
Common Acids (pg 133 in text)
• Hydrochloric HCL
• Sulfuric H2SO4
• Nitric HNO3
• Acetic HC2H3O2
• Phosphoric H3PO4
• Carbonic H2CO3
• Hydrofluoric HF
Empirical Formula and Molecular Formula
CompoundMolecular Formula
EmpiricalFormula
glucose C6H12O6
propane C3H8
butane C4H10
naphthalene C10H8
sucrose C12H22O11
octane C8H18
lowest-termsformula
shows the true numberand type of atoms in a
m’cule
CH2O
C3H8
C2H5
C5H4
C12H22O11
C4H9
Traditional System of Nomenclature
…used historically (and still some today) to name compounds w/multiple-charge cations
To use: 1. Use Latin root of cation.
2. Use -ic ending for higher charge; -ous ending for lower charge.
3. Then say name of anion, as usual.
Element Latin root -ic -ous
gold, Au aur- Au3+
Au1+
lead, Pb plumb- Pb4+
Pb2+
tin, Sn stann- Sn4+
Sn2+
copper, Cu cupr- Cu2+
Cu1+
iron, Fe ferr- Fe3+
Fe2+
Write formulas: cuprous sulfide
auric nitrite
ferrous fluoride
Write names: Pb3P4
Pb3P2
Sn(OH)4
Cu1+ S2– Cu2S
Au3+ NO21– Au(NO2)3
Fe2+ F1– FeF2
cuprous sulfide
auric nitrite
ferrous fluoride
Pb3P4
Pb3P2
Sn(OH)4
Pb? P3– Pb? Pb?
Pb? Pb? Pb?
P3– P3– P3–
P3– P3– Pb2+
Pb4+
Pb2+
Pb4+ Pb4+
plumbic phosphidePb2+
plumbous phosphide
OH1– Sn4+ Sn? OH1– OH1–
OH1–
stannic hydroxide
In insulators (like wood),the v.e– are attachedto particular atoms.
Metallic Bonds
In metals, valence shells of atoms overlap, so v.e– are free to travel between atoms through material.
Not so in metals.
All due to free-moving
v.e–.
Properties of Metals
ductile conduct heat and electricity
malleable